Gas Expansion and Compression: Solving for Volume and Pressure Changes

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SUMMARY

The discussion centers on the application of Boyle's Law (V1P1 = V2P2) to understand gas expansion and compression in a scenario where a 0.5m³ cylinder fills a 5m³ balloon. Participants emphasize that gases can be stored at high pressures in metal cylinders, which allows for significant volume expansion when pressure is reduced. The conversation highlights the importance of understanding pressure differentials and the limitations of balloon materials compared to metal cylinders. Ultimately, the work done by the balloon during inflation is equated to the work done by the gas in the cylinder, leading to further exploration of pressure and volume relationships.

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  • Understanding of Boyle's Law and its mathematical formulation
  • Knowledge of gas laws and pressure-volume relationships
  • Familiarity with concepts of work done in thermodynamics
  • Basic principles of material science regarding elasticity and limits of materials
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  • Study the implications of Boyle's Law in real-world applications
  • Explore the properties of gases under varying pressure conditions
  • Investigate the mechanical properties of balloon materials and their limits
  • Learn about the work-energy principle in thermodynamics
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Ronaldo95163
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The first two are the forces questions with my attempt at them...however I don't have the solutions for them and I wanted to know if what I did was correct.

wrt to the gas questions I'm referring to part e


How can a cylinder with only 0.5m^3 fill a balloon to 5m^3

what I was going to do was use the equation for Boyle's law which is V1P1 = V2P2 and use V2 as difference between the volume in the cylinder and the balloon but seeing that the volume in the cylinder is smaller I started questioning that method... :/
 

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Ronaldo95163 said:
How can a cylinder with only 0.5m^3 fill a balloon to 5m^3

what I was going to do was use the equation for Boyle's law which is V1P1 = V2P2 and use V2 as difference between the volume in the cylinder and the balloon but seeing that the volume in the cylinder is smaller I started questioning that method... :/

Why? Don't you realize that gases can be stored at very high pressure in metal cylinders?
 
But if the cylinder has a volume of 0.5m^3 how can it inflate an empty balloon to 5m^3?
 
Is the pressure in the balloon after it is inflated equal to the pressure of the gas in the cylinder?
 
The question didn't say...only thing that was the same was the temperature
 
Think. Is it reasonable to assume that a balloon could withstand being at the same pressure as a gas in a metal cylinder? Why wouldn't gases be stored in balloons instead of metal cylinders?
 
No
The material of the balloon would expand past its elastic limit and it would burst
 
still not getting it :/
 
Go back and ponder Boyle's Law some more. What happens to the volume of a gas originally kept at a high pressure if the pressure is reduced?
 
  • #10
The volume increases

would the work done by the balloon be equal to the work done by the gas in the metal cylinder??

so

(VΔP) of balloon = V(P2-P1) of the cylinder
 
Last edited:

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